Name: __________________________ Date: _____________ 1. In an ionic compound of formula MmXn, the metal (M) occupies a face-centered cubic lattice and the anions occupy four positions inside the unit cell. Determine the formula of the compound. A) MX B) MX2 C) M2X D) MX3 E) M3X 2. Which one of the following is not a property of gases? A) particles in definite positions B) relatively low densities C) fills any container completely D) expand upon heating E) easily compressed 3. Give the systematic name for the following binary compound: S2F10 A) Disulfur decafluoride B) Sulfur fluoride C) Sulfur decafluoride D) Disulfur pentafluoride E) Disulfur fluoride 4. Which one of the following is not one of the hypotheses of Dalton's atomic theory? A) Atoms are composed of protons, neutrons, and electrons. B) All atoms of a given element are identical; the atoms of different elements are different and have different properties. C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions. D) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. E) Each element is composed of extremely small particles called atoms. Page 1 5. What is the molar mass (g/mol) of sodium sulfite? A) 126.05 B) 142.05 C) 119.05 D) 103.05 E) 149.03 6. Ammonia reacts with oxygen gas to form nitric oxide (NO) and water vapour as follows: 4NH3 + 5O2 → 4NO + 6H2O What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react? A) 1.88 mol B) 1.56 mol C) 3.52 mol D) 3.91 mol E) 2.35 mol 7. Ethylene (C2H4), can be prepared by heating hexane (C6H14) at high temperature. C6H14 C2H4 + other products (assume the equation is already balanced). If the percent yield of ethylene is 42.5 %, what mass of hexane must be used to produce 481 g of ethylene? A) 3.48 x 103 g B) 1.13 x 103 g C) 2.33 x 102 g D) 2.83 x 102 g E) 3.36 x 104 g Page 2 8. A metal, M, was converted to the sulfate, M2(SO4)3. Then a solution of the sulfate was treated with barium chloride to give BaSO4 as follows: M2(SO4)3(aq) + 3BaCl2(aq) → 2MCl3(aq) +3BaSO4(s) If 1.200 g of the metal gave 6.026 g of BaSO4, what is the identity of the metal? A) Ga B) Ni C) Fe D) Cr E) In 9. You mix 25.0 mL of 0.234 M FeCl3 with 42.5 mL of 0.453 M NaOH. What is the molar concentration of the excess reactant remaining in solution? A) 0.025 M NaOH B) 0.0017 M NaOH C) 0.0017 M FeCl3 D) 0.0023 M FeCl3 E) 0.023 M FeCl3 10. Which of the following is/are weak electrolyte(s) in aqueous solution? I. CH3COOH II. HF III. NH3 A) All of them B) I only C) I and II only D) I and III only E) II only 11. Which of the following has/have resonance structures? - I. SO3 II. C2H4 III. NO2 A) I and III only B) I only C) II and III only D) I and II only E) All of them Page 3 12. Rank the following compounds in order of increasing Lattice Energy. BaSe MgO CaS A) BaSe < CaS < MgO B) BaSe < MgO < CaS C) CaS < MgO < BaSe D) MgO < CaS < BaSe E) CaS < BaSe < MgO 13. How many protons and electrons are present in the Se2- ion? A) 34 protons and 36 electrons B) 79 protons and 81 electrons C) 34 protons and 32 electrons D) 79 protons and 77 electrons E) 34 protons and 34 electrons 14. .Which one of the following elements has the largest first ionization energy? A) Cl B) Ca C) Se D) Te E) Ga 15. The electronic configuration of a ground–state Chromium (Cr) is A) [Ar]4s13d5 B) [Ar]4s23d4 C) [Ne]4s23d7 D) [Ne]4s13d6 E) [Ar]4s24d7 16. Which statement about electromagnetic radiation is false? A) As wavelength increases, energy increases. B) As frequency increases, wavelength decreases. C) As wavelength increases, frequency decreases. D) Wavelength and frequency are inversely proportional. E) Wavelength and energy are inversely proportional. Page 4 17. What is the height of a column of methyl alcohol that will be supported by one atmospheric pressure? The density of methyl alcohol is 0.787 g/cm3. [1 Pa = 1 kg/m·s2 and 1 atm = 101325 Pa; gravitational constant = 9.80665 m/s2] A) 13.1 m B) 10.3 m C) 7.87 m D) 9.80 m E) 12.3 m 18. At 40.0 C a sample of nitrogen gas exerts a pressure of 2.2 atm. What is the pressure when the volume of the gas is reduced to one-fifth of the original value at the same temperature? A) 11 atm B) 10. atm C) 2.2 atm D) 4.4 atm E) 5.0 atm 19. Analysis of a volatile liquid shows that it contains 62.04% carbon, 10.41% hydrogen, and 27.54% oxygen by mass. At 150.°C and 1.00 atm, 500. mL of the vapor has a mass of 0.8365 g. What is the molecular formula of the compound? A) C3H6O B) C6H12O2 C) C12H24O4 D) C4H6O E) C2H5OH 20. Consider the following reaction (at STP) and identify the false statement. C2H2(g) + N2(g)→ 2HCN(g) A) Producing exactly 22.4 L of HCN requires the complete reaction of 28 g of N2. B) This is a combination reaction. C) 26 g of C2H2 react to yield 44.8 L of HCN. D) 22.4 L of C2H2 react to yield 44.8 L HCN. E) 22.4 L of N2 react to yield 44.8 L HCN. Page 5 21. The average kinetic energy of ideal gas molecules is directly proportional to the ____. A) absolute temperature of the sample B) density of the sample C) mass of the molecule D) pressure of the sample E) volume of the sample 22. What is the molar mass of an unknown gas, which effuses with a rate equal to one third (1/3) the rate of helium gas? A) 36 g/mol B) 72 g/mol C) 18 g/mol D) 54 g/mol E) 92 g/mol 23. Which of the following is the correct approach to prepare a 100.0 mL of a 1.00 M H2SO4 solution from a 10.0 M H2SO4 stock solution? A) Add 10.0 mL of the stock solution to 80.0 mL of H2O, stir and dilute to 100.0 mL. B) Add 50.0 mL of the stock solution to 25.0 mL of H2O, stir and dilute to 100.0 mL C) Add 25.0 mL of the stock solution to 50.0 mL of H2O, stir and dilute to 100.0 mL. D) Add 90.0 mL of stock solution to 10.0 mL of H2O and stir the solution. E) Add 1.0 mL of the stock solution to 99.0 mL of H2O and stir the solution. 24. Consider the combustion of hydrogen given below: H2(g) + ½ O2(g) → H2O(g) ΔH = -241.8 kJ/mol What is the enthalpy change, in kJ, when the reaction is started with 52.5 g of H2 and 52.5 g of O2 ? A) -793 kJ B) -537 kJ C) -192 kJ D) -645 kJ E) -564 kJ Page 6 25. If the internal energy of a system decreases by 135 J and at the same time it absorbs 24 J of heat, what is the work? A) -159 J B) 111 J C) -111 J D) 213 J E) 159 J 26. According to the VSEPR model, the predicted molecular geometries of Ammonia (NH3), Hydrogen cyanide (HCN) and Phosphorus pentachloride (PCl5) respectively are A) trigonal pyramidal, linear and trigonal bipyramidal. B) trigonal planar, linear and trigonal pyramidal. C) trigonal pyramidal, bent and trigonal bipyramidal. D) tetrahedral, linear and octahedral. E) linear, bent and trigonal bipyramidal. 2– 27. According to the VSEPR model, what is the predicted F–Si–F bond angle in SiF6 ? A) 90° B) 109.5° C) 120° D) 145° E) 130° 28. How many π and σ bonds are there in the molecule shown below? A) 3 π and 18 σ B) 2 π and 16 σ C) 3 π and 15 σ D) 2 π and 19 σ E) 3 π and 10 σ Page 7 29. What is the total number of electron domains around the central atom in XeF2 ? A) 5 B) 2 C) 3 D) 4 E) 6 30. What diatomic molecule and/or ion(s) would have the molecular orbital electron configuration given below? 2 * 2 2 * 2 2 1 1s 1s 2s 2s 2py 2pz + – A) C2 and B2 – + B) C2 and N2 – + C) C2 and B2 + D) N2 and C2 + E) O2 and N2 - 31. Indicate the type of hybrid orbitals used by the central atom in ClBr2 . A) sp3d B) sp2 C) sp D) sp3 E) sp3d2 32. What is the molality of 8.6% glucose (C6H12O6) by mass in water? A) 0.52 m B) 0.32 m C) 0.34 m D) 0.44 m E) 0.67 m Page 8 33.